# Assuming equal concentrations and complete dissociation, rank these aqueous solutions by their freezing points. CoCl3 K2CO3 KNO3

49,611 results
1. ## chemistry

Arrange the following aqueous solutions in order of decreasing freezing points (lowest to highest temperature): 0.10 m Na3PO4, 0.35 m NaCl, 0.20 m MgCl, 0.15 m C6H12O6 and 0.15 m CH3COOH.

2. ## chemistry

Arrange the following aqueous solutions in order of increasing freezing points (lowest to highest temperature): 0.10 m glucose, 0.10 m BaCl2, 0.20 m NaCl, and 0.20 m Na2SO4.

3. ## Chemistry

Solutions of potassium carbonate, copper(II) chloride, and lead(II) nitrate are each added to a beaker. Will any compound(s) precipitate from solution? Write a balanced net ionic equation for any precipitation reaction that occurs. I have gotten this so

4. ## Chemistry

Assuming equal concentrations , rank these solutions by pH. RbOH(aq), NH3(aq), HF(aq) HBr(aq), Ca(OH)2(aq). I know the most acidic solution has the lowest pH and the most basic solution has the highest pH. But how am i supposed to know the pH if i don't

5. ## Chemistry

Assuming equal concentrations and complete dissociation, rank these aqueous solutions by their freezing points. CoCl3 K2CO3 KNO3

6. ## chemistry

help please?? Assuming 100% dissociation, calculate the freezing point and boiling point of 2.64 m K3PO4(aq). Tf= Tb=

7. ## Chemistry

Aqueous solutions of copper (II) sulfate, CuSO4, and potassium carbonate, K2CO3, a blue parcipitate of copper (II) carbonate forms in addition to one other compound. We have to write the balanced chemical equation for that but our teacher didn't teach us

8. ## CHEMISTRY

Assuming equal concentrations, rank these aqueous solutions by their freezing point: LiSO4, Li3PO4, SnCl4, NH4Br. (from highest freezing point to lowest freezing poinT) Thanks.

9. ## chemistry

Which of the following pairs of aqueous solutions will react when mixed? K2CO3 + HNO3 HCl + LiOH MgCl2 + KOH Li2S + HCl All of these solution pairs will produce reactions.

10. ## Chemistry

What are the concentrations of OH– and H in a 0.00070 M solution of Ba(OH)2 at 25 °C? Assume complete dissociation.

11. ## chemistry

Assuming equal concentrations, rank these aqueous solutions by their freezing point.? K2CO3, Li3PO4, Sn(ClO3)4, NH4I I tried to rank them according to the number of ions but i can't get it. highest freezing point --> lowest freezing point Sn(ClO3)4 ->

12. ## Chemistry

Assuming equal concentrations, rank these aqueous solutions by their freezing point: low to high NH4Cl, Sn(ClO3)4, Na2SO4, and AlBr3.

13. ## Chemistry

Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at -14.5 degrees celcius ? The freezing point for pure water is 0.0 degrees celcius and Kf is equal to 1.86 degrees

14. ## Chemistry

Assume equal concentrations, rank these solutions by pH HBrO, Ca(OH)2, HCl, KOH, NH3 Here's how I ranked it: highest: Ca(OH)2 > HCl > KOH > NH3 > HBrO lowest is this correct? if not please tell me why!

15. ## chem

what are the normal freezing points and boiling points of the following solutions: a. 21.1g NaCl in 135mL of water b. 15.4g urea in 66.7 mL water?

16. ## chemistry

Assuming equal concentration rank these by freezing points, Na3PO4, Li2Co3,NH4Cl, and Sn(NO3)4

17. ## Chemistry hw

Assuming 100% dissociation, calculate the freezing point and boiling point of 3.13 m SnCl4(aq). Tf=? Tb=? My work: SnCl4 with 100% dissociation gives a van't hoff factor of 5, 1Sn 4+ ion and 4 Cl- ions deltaT = i x Kf x m for freezing point = 5 x 0.51C/m x

18. ## Chemistry

Which one of the following pairs of 0.100 mol L-1 solutions, when mixed, will produce a buffer solution? A. 50. mL of aqueous CH3COOH and 25. mL of aqueous CH3COONa B. 50. mL of aqueous CH3COOH and 25. mL of aqueous HCl C. 50. mL of aqueous NaOH and 25. mL

19. ## AP chemistry

which of the following aqueous solutions should not form a precipitate with aqueous ba(no3)? 1. KOH 2. K2CO3 3. K2SO4 4. K3PO4

20. ## Chemistry

assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at -14.5 C? The freezing point for pure water is 0.0 C and is equal to 1.86 C/m .

21. ## chemistry

Assuming 100% dissociation, calculate the freezing point and boiling point of 0.700 mol of AgNO3 in 1.00 kg of water.

22. ## AP Chem

1. Van't Hoff factors depend on the concentrations of the dissolved solute species. Why would a dilute solution have a Van't Hoff factor closer to the ideal value? a. because in dilute solutions solute species are less likely to bump into each other and

23. ## Chemistry

Assuming equal concentrations and complete dissociation, rank these aqueous solutions by their freezing points: Li2SO4 K3PO4 LiNO3

24. ## chemistry

Which of the following aqueous solutions should NOT form a precipitate with aque- ous Ba(NO3)2? 1. K3PO4 2. K2SO4 3. K2CO3 4. KOH

25. ## Chemistry

What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that is buffered at a pH of 4.84 and has a freezing point of -2.0 ∘C? (Assume complete dissociation of sodium benzoate and a density of 1.01 g/mL for the solution.)

26. ## Chemistry

Arrange the following aqueous solutions in order of increasing boiling point, explain your answer: 0.120 m glucose (C6H12O6), 0.05 m LiBr, 0.05 m Zn(NO3)2. Using data the boiling point constants given in the test book, calculate the boiling points of each

27. ## chemistry

which of the following liquids have the highest freezing point? a- aqueous Fe(NO3)3 (0.030) b- aqueous glucose (0.050 m) c- aqueous NaI (0.030 m) d- aqueous NaI (0.010 m) e- pure water please explain the concept behind it as well thank you!

28. ## Chemistry

Which one of the following liquids will have the highest freezing point? A. pure H2O B. aqueous glucose (0.050 m) C. aqueous CoI2 (0.030 m) D. aqueous FeCl3 (0.030 m) E. aqueous NaI (0.030 m) Could you please give a step by step process?

29. ## chemistry

What is the expected van't Hoff factor for NaC2H3O2 in an aqueous solution, assuming 100% dissociation.

30. ## Chemistry

Consider this reaction: 3 K2CO3 (aq) + 2 CrCl3 (aq) -> Cr2(CO3)3 (s) + 6 KCl (aq) If 1.2 moles of CrCl3 react, how many moles of K2CO3 will react with it? A. 0.80 mol K2CO3 B. 1.2 mol K2CO3 C. 1.8 mol K2CO3 D. 2.4 mol K2CO3 I'm not sure where to even

31. ## Chemistry

Assuming 100% dissociation, calculate the freezing point and boiling point of 1.96 m SnCl4 (aq)

32. ## Chemisrty

Assuming equal concentrations, rank these solutions by pH: hclo4 caoh2 NH3 koh hbro

33. ## science

When substances such as sugar and table salt are dissolved in water, the freezing points of the new solutions are lower than the freezing point of water. Also, the more material dissolved, the lower the freezing point. The boiling points of these

34. ## Chemistry

Assuming complete dissociation, what is the pH of a 2.55 mg/L Ba(OH)2 solution?

35. ## Chem

Assuming 100% dissociation, calculate the freezing point and boiling point of 2.45 m Na2SO4(aq). Constants may be found here sites. google. com/site/chempendix/colligative.

36. ## Chemistry

Assuming 100% dissociation, calculate the freezing point and boiling point of 2.45 m Na2SO4(aq). Constants may be found here sites. google. com/site/chempendix/colligative.

37. ## chemistry

How do you arrange these aqueous solutions in order of decreasing freezing point: 0.10 m Na3PO4, 0.35 m NaCl, 0.20 m MgCl2, 0.15 m C6H12O6, and CH3OOH?

38. ## Chemistry

1) For a freezing point depression experiment we had to create an ice bath and add salt to the ice. I have to answer the question, why was salting the ice necessary in order to complete the experiment and how does this apply to the principles/concepts

39. ## Chemistry

Write the formulas of the ions (including charges) present in aqueous solutions of the following: K2CO3 NH4NO3 NA2Cr2O7 Mg(C2H3O2)2 Make sure it is both mass and charge balanced. Here is a listing of many polyatomic ions. This should give you a start. Post

40. ## chem

Assuming complete dissociation, what is the molality of an aqueous solution of KBr whose freezing point is -2.95 ∘C? The molal freezing-point-depression constant of water is 1.86 (∘C⋅kg)/mol. Molality = m

41. ## Chemistry

Assume equal aqueous concentrations of each of the following substances. Which has the lowest freezing point? C2H12O6 CH3OH C12H22O11 NaOH i say its NaOH am i right ?

42. ## Chemistry

Determine the freezing points of each 0.20m aqueous solution. a)K2SO4 b)CsNO3 c)Al(NO3)3

43. ## chem101

Which of the following solutes in aqueous solution would be expected to exhibit the LARGEST freezing-point lowering (assuming ideal behavior)? A. 0.1 m NaCl B. 0.2 m CH3COOH C. 0.1 m MgCl2 D. 0.05 m Al2(SO4)3 E. 0.25 m NH3

44. ## science

When substances such as sugar and table salt are dissolved in water, the freezing points of the new solutions are lower than the freezing point of water. Also, the more material dissolved, the lower the freezing point. The boiling points of these

45. ## Chemistry

Calculate the freezing point of the following solutions, assuming complete dissociation.3.7% KCL by mass (in water)

46. ## Chemistry

Assuming complete dissociation of the solute, how many grams of KNO_3 must be added to 275mL of water to produce a solution that freezes at -14.5C? The freezing point for pure water is 0.0 C and K_f is equal to 1.86 C. Delta T= Kf*m*i i=2 m=3.90 solvent

47. ## Moorpark

Determine the concentration of NO3- in each of the following aqueous solutions. (Assume complete dissociation of each compound.) 0.30 M KNO3, 0.30 M Ca(NO3)2, 0.30 M Cr(NO3)3

48. ## Re chemistry

What are the concentrations in mass of the following solutions: a) a 200mL aqueous solution containing 4.26g sodium solfate. b) a 2.00 L aqueous solution containing 107.0g ammonium chloride NH4Cl. Plz can give me someone the answers for BOTH and the steps

49. ## Chem 2

Assuming 100% dissociation, calculate the freezing point and boiling point of 2.44 m Na2SO4(aq)

50. ## Chemistry

Given that the vapor pressure of water is 17.54 Torr at 20 °C, calculate the vapor-pressure lowering of aqueous solutions that are 1.90 m in (a) sucrose, C12H22O11, and (b) aluminum chloride. Assume 100% dissociation for electrolytes. I got .5799 Torr for

51. ## science

When substances such as sugar and table salt are dissolved in water, the freezing points of the new solutions are lower than the freezing point of water. Also, the more material dissolved, the lower the freezing point. The boiling points of these

52. ## science

Using data from this table of molal boiling-point-elevation and freezing-point-depression constants, calculate the freezing and boiling points of each of the following solutions. a)0.39 m glucose in ethanol (b) 22.8 g of decane, C10H22, in 53.9 g CHCl3 (c)

53. ## finding boiling points of solutions

What is the boiling point (in degrees Celsius ) of each of the solutions below? For water, Kb = 0.51 (Degrees C * kg)/mol The vapor pressure of water at 45.0C is 71.93 mm Hg. 1. A solution of 15.0g of urea, CH4N2O, in 164 g of water at 45.0 degrees C. For

54. ## science

four flasks each contain 100 milliliters of aqueous solutions equal concentrations at 25 degress C and 1 atm. the four flasks are KCL,CH3OH, Ba(OH)2, and CH3COOH. the question is Which solution had the lowest freezing point and explain answer

55. ## Chemistry

what is the freezing point of 16.7g of LiCl in 136g of water, assuming complete dissociation for water kf= -1.86/mol

56. ## Chemistry

what is the freezing point of 16.7g of LiCl in 136g of water, assuming complete dissociation for water kf= -1.86/mol

57. ## Hayden

Chloroacetic acid has a relatively large equilibrium constant, so at low acid concentrations it is necessary to use the quadratic equation in order to calculate the concentrations of the aqueous species. Ka for ClCH2COOH is 1.4 ´ 10-3. For the problems

58. ## AP Chemistry

Nitric acid is a strong acid. Does this mean that a) HNO3 dissociates completely to H+ (aq) and NO3 ^1- (aq) when it dissolves in water OR b) aqueous solutions of HNO3 contain equal concentrations of H+(aq) and OH- (aq) Thank you!

59. ## Chemistry

What are the concentrations of the following solutions: a) a 200mL aqueous solution containing 4.26g sodium solfate. b) a 2.00 L aqueous solution containing 107.0g ammonium chloride NH4Cl. Plz can give me someone the answers for BOTH and the steps how you

60. ## chemistry

(7 points) 1. The reaction that you just witnessed in while doing your titration was: HCl + NaOH  H2O + NaCl. This equation is balanced. Your unknown solutions contained HCl solutions of unknown concentrations, and your titrant was a 0.75 M solution of

61. ## Chemistry

Calculate the boiling points of freezing points of the following solutions in water. a) boiling point of a 2.25m solution of propylene glycol (a non-electrolyte) b)freezing point of a 1.0m solution of potassium iodide c)freezing point of a 1.0m solution of

62. ## chemistry

this is a really long question. i don't understand how to answer it. help please. A 10.0% aquueous solution of sulfuric acid has a density of 1.0661 g/mL at 20 degrees celsius. A. how many grams of H2SO4 are found in 50.0 g of this solution? B. how many

63. ## Conductivity

Complete the table below: For each of the following sets pick the compound with the highest conductivity in a 1 M aqueous solution. (Enter the number at the top of the column containing the correct answer.) 1 2 3 Answers a HCl HC2H3O2 H2PO4– b KNO3

64. ## math

Consider an equilateral triangle with points located at each vertex and at each midpoint of a side. (See picture.) This problem uses the set of numbers {1, 2, 3, 4, 5, 6}. Place one number at each point. Call the sum of the three numbers along any one side

65. ## chem

Rank these in order of increasing freezing points: C2H6O, NaCl, NaSO4, C12H22O11 I suggest that you look them up. You will have to make an assumption at the isomer of the organic compounds that is intended, but it will not make a difference to the ranking.

66. ## College Math

For questions 1-2, apply the quadratic formula to find the roots of the given function, and then graph the function. 1. f(x) = x2 + 4 (6 points) g(x) = x2 - x – 12 For questions 3-4, factor the quadratic expression completely, and find the roots of the

67. ## chemistry

Calculate the freezing point of 0.15 m calcium chloride aqueous solution. Assume that the molal freezing point depression constant of water is 1.86°C·kg/mol and that the freezing point of water is 0.00°C

68. ## chem hw

Assuming equal concentrations, rank these aqueous solutions by their freezing point: Li2SO4, Li3PO4, SnCl4, NH4Br. (from highest freezing point to lowest freezing poinT) Is the order Li3PO4, Li2SO4, SnCl4, and NH4Br???????? If not what is the correct

69. ## CHEMISTRY

Assuming equal concentrations , rank these solutions by pH. RbOH(aq), NH3(aq), HF(aq) HBr(aq), Ca(OH)2(aq).

70. ## Chemistry

Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at -14.5 C? The freezing point for pure water is 0.0 C and Kf is equal to 1.86 C/m. * Use Tf = Kf*i*m

71. ## chemistry

assuming complete dissociation of the solute, how many grams of \rm KNO_3 must be added to 275 \rm mL of water to produce a solution that freezes at -14.5 ^\circ {\rm C}? The freezing point for pure water is 0.0 ^\circ {\rm C} and K_f is equal to 1.86

72. ## Chemistry AP

What are the concentrations of benzoic acid and sodium benzoate in a solution that is buffered with a pH of 4.55 and has a freezing point of -2.0 degrees Celsius? (assume complete dissociation and a density of 1.01g/mL for the solution.)

73. ## CSU

what is the freezing point of 16.7g of LiCl in 136g of water, assuming complete dissociation for water kf= -1.86/mol

74. ## Chemistry

what is the freezing point of 16.7g of LiCl in 136g of water, assuming complete dissociation for water kf= -1.86/mol

75. ## Chemistry

what is the freezing point of 16.7g of LiCl in 136g of water, assuming complete dissociation for water kf= -1.86/mol

76. ## Chemistry

Suppose you had a 1.00 m solution of AlCl3. Assuming complete dissociation, what is the theoretical change in the freezing point of this solution?

77. ## Chemistry

The ionisation of water plays an important role in the equilibria of aqueous solutions. Kw= 1.008 x 10-14 mol2 dm-6 at 298K. (a) Calculate the pH of the following solutions at 298K showing all your working. Assume full dissociation in each case. (i) 0.054

78. ## Chemistry

What should the molar concentrations of benzoic acid and sodium benzoate be in a solution that is buffered at a pH of 4.75 and has a freezing point of -2.0 ∘C? (Assume complete dissociation of sodium benzoate and a density of 1.01 g/mL for the solution.)

79. ## intro to chem

disolving sucrose, NaCl< and calcium chloried affect the boiling point of frezing point of water. Assuming that you have 0.1m solution of all these 3 compounds: a)rank then in order of decreasing freezing point. b) rank in order of increasing boiling point

80. ## chem

calculate the freezing and boiling points of each of the following solutions. (a) 0.50 m glucose in ethanol for the freezing point i got 58 but it said i have the wrong sign...?

81. ## chemistry

Nitric acid is a strong acid. Does this mean that a) HNO3 dissociates completely to H+ (aq) and NO3 ^1- (aq) when it dissolves in water OR b) aqueous solutions of HNO3 contain equal concentrations of H+(aq) and OH- (aq) Thank you!

82. ## Chemistry

1) it is found that .30 M solutions of the three shots Na3X, Na2Y and NaZ have pH's of 8.5, 7.0 and 10.5 not necessarily in order. (X,Y, and Z AE anions. Na is sodium ion) A) explain how anions can act as bases in aqueous solution. Write a chemical

83. ## Chemistry

Assuming complete dissociation, what is the pH of a 3.73 mg/L Ba(OH)2 solution?

84. ## chemistry

I have this on my homework but cannot fine any examples in the book or my notes that relate to a problem set up this way, can you help? What are the concentrations of OH– and H in a 0.00078 M solution of Ba(OH)2 at 25 °C? Assume complete dissociation.

85. ## Chem TWO

Assuming 100% dissociation, calculate the freezing point and boiling point of 2.91 m K3PO4(aq).

86. ## Chemistry

Calculate the pH and of aqueous solutions having the fol lowing ion concentrations a. [H^ + ]=1.0*10^ -14 M b. [OH^ - ]=5.6*10^ -8 C. [H^ + ]=2.7*10^ -3 M d. [OH^ - ]=0.061M

87. ## Chemistry

Which aqueous solution below is expected to have the lowest freezing point? Assume 100% dissociation for ionic species. 1)0.25m MgBr2 2)0.30m Na2SO4 3) 0.50m KCl 4) 1.0m sucrose 5) 0.40m Cr(NO3)3 I think that the answer is 0.30NaSO4 but I am not positive.

88. ## chemical and ionic equlibrium

1. calculate H+ ion concentrates in 0.10 m acetic acid solutions. Given that dissociation constant of acetic acid in water is 1.8 * 10^-5 ? 2. Calculate the concentration of H+ and OH- in a 0.05 m HNO3 solutions at 25^0c ? 3. The degree of dissociation of

89. ## Chemistry

calculate the freezing and boiling points of each of the following solutions. (a) 0.37 m glucose in ethanol freezing point ______I got -1.2e2 but its wrong_______°C boiling point _________I got 1.1e2 but its wrong:(____°C (b) 15.0 g of decane, C10H22, in

90. ## math,correction

Find four solutions for the equation 3x+5y=15 so the equation will turn to be y=-(3)/(5)x+ (3) and when i do the table i get these points for the solution (-2,4.2),(-1,3.60),(0,3),(1,1.8) ok Let me give you a help. Take the slope, denominator. 5. Now make

91. ## Chemistry

Based on the following observations for 3 unidentified metals (Z, X, and D) and solutions of their metal cations (Zn+ and En+), rank the metals in terms of reducing agent strength, from lowest to highest. -When metal X is placed in an aqueous solution of

92. ## Physical Chemistry

When 1.33 g of a nonpolar solute was dissolved in 50.0 g of phenol, the latter's freezing point was lowered by 1.454°C. Calculate the molar mass of the solute. The kf of phenol is 7.27 (K·kg)/mol. What is the normal boiling point of an aqueous solution

93. ## Punakha central school. Bhutan

Dissociation constand of propanoic acid is 1.76. Determine degree of dissociation of P ropanoic acid in 0.2molar in aqueous solution?

94. ## chemistry

PLEASE SHOW PROCEDURE! You wish to prepare an aqueous solution that has a freezing point of -0.100 degrees Celsius. How many milliliters of 12.0 M HCl would you use to prepare 250.0 mL of such a solution? [Hint: Note that in a dilute aqueous solution,

95. ## chem

what are the normal freezing points and boiling points of the following solutions: a. 21.1g NaCl in 135mL of water b. 15.4g urea in 66.7 mL water?

96. ## Chemistry

Can anyone tell me if I am right on these? Calculate the amount of solute needed to make each of the solutions 225g of 10% (m/m) K2CO3 solution Answer: 22.5g K2CO3 0.50kg of 18% (m/m) KOH solution Answer: 90g KOH

97. ## Chemistry Help

The most effective buffer solutions have equal concentrations of salt and acid (or base). Find the pH of a buffer solution with equimolar concentrations of: (a) HCOOH and NaCOOH (Ka = 3.5 x 10-4 for HCOOH) (b)CH3NH2 and CH3NH3Cl (Kb = 3.7 x 10-4 for

98. ## AP Chem

What mass of K2CO3 is required to clean up a spill of 282 ml of 1.05 M HCl if HCl(aq) reacts with K2CO3 according to 2HCl(aq) + K2CO3(aq) → 2KCl(aq) + CO2(g) + H2O(l)?

99. ## chemistry

What mass of K2CO3 is required to clean up a spill of 339 ml of 2.65 M HCl if HCl(aq) reacts with K2CO3 according to 2HCl(aq) + K2CO3(aq) ¨ 2KCl(aq) + CO2(g) + H2O(l)?

100. ## Chemistry, #5

For propanioic acid, HC3H5O2, Ka=1.3 x 10^-5, determine the concentration of the species present, the pH and the percent dissociation of a 0.21 M solution. Do this for H+, OH-, C3H5O2-, HC3H5O2, and the pH and percent dissociation. If someone can please